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Equilibrium Constant from Nernst Equation

If the standa...

Question

If the standard electrode potential constant for a cell is $2 V$ at $300 K$ the equilibrium constant (K) for the reaction:
$Z n (s) + C u^{2 +} (a q) ⇌ Z n^{2 +} (a q) + C u (s)$ at $300 K$ is approximately.

$(R = 8 J K^{- 1} m o l^{- 1}, F = 96000 C m o l^{- 1})$

e^{160}

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e^{320}

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e^{- 160}

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e^{- 80}

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Solution

The correct option is C $e^{160}$
$Δ G^{o} = - R T l n K = - n F E_{c e l l}^{o}$

$l n K = \frac{n \times F \times E^{o}}{R \times T} = \frac{2 \times 96000 \times 2}{8 \times 300}$

$l n K = 160$

$K = e^{160}$

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